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1.216 g of an organic compound was Kjeldahlised and the ammonia evolved was absorbed in 100 mL of 1-N H_(2)SO_(4). The remaining acid solution was made upto 500 mL by dilution with water. 20 mL of this diluted solution required 32 mL of N//10 NaOH solution for complete neutralisation. calculate the percentage of nitrogen in the compound.

Answer» <html><body><p></p>Solution :Step I. Calculation of the normality of diluted `H_(2)SO_(4)` solution. <br/> Volume of `NaOH` solution = 32 mL <br/> Normality of `NaOH` solution `= N//10` <br/> Volume of the `H_(2)SO_(4)` solution `= 20` mL <br/> Normality of `H_(2)SO_(4)` solution can be calculated by applying normality equation <br/> `ubrace(N_(<a href="https://interviewquestions.tuteehub.com/tag/1-256655" style="font-weight:bold;" target="_blank" title="Click to know more about 1">1</a>)V_(1))_("Acid")= ubrace(N_(2)V_(2))_("Base")` <br/> `Nxx20=1/10xx32, N=32/(10xx20)` <br/> Step <a href="https://interviewquestions.tuteehub.com/tag/ii-1036832" style="font-weight:bold;" target="_blank" title="Click to know more about II">II</a>. Calculation of the volume of unused `H_(2)SO_(4)` <br/> `ubrace(N_(1)V_(1))_("Conc. acid")= ubrace(N_(2)V_(2))_("Diluted acid")` <br/> `1xxV=(32xx500)/(10xx20)=80 mL`. <br/> Step <a href="https://interviewquestions.tuteehub.com/tag/iii-497983" style="font-weight:bold;" target="_blank" title="Click to know more about III">III</a>. Calculation of the volume of used `H_(2)SO_(4)` <br/> Total volume of `H_(2)SO_(4)` yaken = 100 mL <br/> Volume of `H_(2)SO_(4)` unused = 80 mL <br/> Volume of `H_(2)SO_(4)` used `100-80=20` mL. <br/> Step IV. Calculation of the percentage of nitrogen. <br/> Percentage of`(1.4xx"Normality of acid used"xx"Volume of acid used")/("Mass of the compound")` <br/> `=(1.4xx1xx20)/(1.216)=23.03 %`</body></html>


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